Energetics

Megan Thomas
Quiz by Megan Thomas, updated more than 1 year ago
Megan Thomas
Created by Megan Thomas almost 3 years ago
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Description

Year 13 Chemistry Quiz on Energetics, created by Megan Thomas on 10/07/2017.

Resource summary

Question 1

Question
Lattice energy is the energy change when 1mol of an [blank_start]ionic[blank_end] compound is formed from its [blank_start]gaseous[blank_end] ions under [blank_start]standard conditions.[blank_end]
Answer
  • ionic
  • gaseous
  • standard conditions

Question 2

Question
Values of lattice energy are
Answer
  • always positive
  • always negative
  • can be negative or positive

Question 3

Question
Enthalpy change of atomisation is the enthalpy change when 1mol of gaseous ions is formed from the [blank_start]element[blank_end] in its [blank_start]standard state.[blank_end]
Answer
  • element
  • standard state.

Question 4

Question
First electron affinity is the enthalpy change when one [blank_start]e-[blank_end] is added to each [blank_start]gaseous[blank_end] atom in 1 mol to form 1 mol of -1 gaseous [blank_start]ions[blank_end].
Answer
  • e-
  • gaseous
  • ions

Question 5

Question
What are the factors that affect lattice enthalpy?
Answer
  • Charge on the ions
  • Amount of ions present
  • Temperature
  • Radius of the ions

Question 6

Question
The [blank_start]higher[blank_end] the charge on the ion the [blank_start]higher[blank_end] the lattice enthalpy.
Answer
  • higher
  • lower
  • higher
  • lower

Question 7

Question
Enthalpy of hydration is the [blank_start]heat[blank_end] change when 1 mol of gaseous ions completely dissolve in [blank_start]water.[blank_end]
Answer
  • heat
  • water

Question 8

Question
Label the Born Haber Cycle with the process occurring at each stage.
Answer
  • Lattice Enthalpy
  • 1st Electron Affinity
  • Enthalpy of Atomisation
  • 1st Ionisation Energy
  • 2nd Ionisation Energy
  • Lattice Enthalpy
  • 1st Electron Affinity
  • Enthalpy of Atomisation
  • Enthalpy of Formation
  • 1st Ionisation Energy
  • 2nd Ionisation Energy
  • Enthalpy of Formation
  • Lattice Enthalpy
  • 1st Electron Affinity
  • Enthalpy of Atomisation
  • 1st Ionisation Energy
  • 2nd Ionisation Energy
  • Enthalpy of Formation
  • Lattice Enthalpy
  • 1st Electron Affinity
  • Enthalpy of Atomisation
  • 1st Ionisation Energy
  • 2nd Ionisation Energy
  • Enthalpy of Formation
  • Lattice Enthalpy
  • 1st Electron Affinity
  • Enthalpy of Atomisation
  • 1st Ionisation Energy
  • 2nd Ionisation Energy
  • Enthalpy of Formation
  • Lattice Enthalpy
  • 1st Electron Affinity
  • Enthalpy of Atomisation
  • 1st Ionisation Energy
  • 2nd Ionisation Energy
  • Enthalpy of Formation

Question 9

Question
[blank_start]Enthalpy of Solution[blank_end] is the heat change when 1 mol of an ionic substance dissolves in water
Answer
  • Enthalpy of Solution

Question 10

Question
An ionic lattice dissloves in water because water molecules disrupt the attraction between [blank_start]cations[blank_end] and [blank_start]anions[blank_end] in the lattice. Cations become surrounded by the [blank_start]negative[blank_end] part of the water molecules. Anions become surrounded by the [blank_start]positive[blank_end] part of the water molecules.
Answer
  • cations
  • anions
  • negative
  • positive

Question 11

Question
Enthalpy of Hydration is ...
Answer
  • always positive
  • always negative
  • sometimes positive, sometimes negative

Question 12

Question
Entropy is the measure of the [blank_start]disorder[blank_end] of a [blank_start]system[blank_end].
Answer
  • disorder
  • system

Question 13

Question
A disorder increases entropy...
Answer
  • decreases
  • increases
  • can't tell
  • is unchanged

Question 14

Question
Entropy decreases as the solid becomes more complex.
Answer
  • True
  • False

Question 15

Question
Entropy [blank_start]increases[blank_end] from solid to liquid to gas because molecules become [blank_start]more disordered[blank_end].
Answer
  • increases
  • more disordered

Question 16

Question
There is only a small jump in entropy from ice to water despite the state change as the [blank_start]hydrogen bonding[blank_end] means water is still relatively [blank_start]ordered[blank_end].
Answer
  • hydrogen bonding
  • ordered

Question 17

Question
Which factors cause a change in entropy
Answer
  • temperature change
  • addition of a catalyst
  • change in volume
  • number of gas molecules
  • state change
  • concentration change

Question 18

Question
If Gibbs Free Energy is 0 this means
Answer
  • the substance is an element or the reaction is at equilibrium
  • the reaction is spontaneous
  • work must be supplied from the surroundings for the reaction to occur

Question 19

Question
If Gibbs Free Energy is less than 0 this means...
Answer
  • the substance is an element or the reaction is at equilibrium
  • the reaction is spontaneous
  • work must be supplied from the surroundings for the reaction to occur

Question 20

Question
If Gibbs Free Energy is greater than 0 this means...
Answer
  • the substance is an element of the reaction is at equilibrium
  • the reaction is spontaneous
  • work must be supplied from the surrounding for the reaction to occur

Question 21

Question
If delta (the little triangle symbol) G is negative delta S must be [blank_start]positive[blank_end] and delta H [blank_start]negative[blank_end]. The reaction will be spontaneous.
Answer
  • positive
  • negative

Question 22

Question
If total entropy is positive the reaction is [blank_start]feasible[blank_end].
Answer
  • feasible

Question 23

Question
total entropy = entropy of [blank_start]surroundings[blank_end] + entropy of [blank_start]system[blank_end]
Answer
  • surroundings
  • system
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